chapter 4€¦ · dalton’s atomic theory section 4.3 copyright © cengage learning. all rights...

Chapter 4(part 1)

Chemical Foundations: Elements, Atoms, and Ions

Copyright © Cengage Learning. All rights reserved 1

The Elements

Section 4.1


• 118 known: 88 found in nature, others are made in laboratories.

• Just as you had to learn the 26 letters of the alphabet before you learned to read and write, you need to learn the names and symbols of the chemical elements before you can read and write chemistry.

The Elements

Section 4.1


The Elements

Section 4.1


• Could mean a single atom of an element (Ar or H).

• Could mean molecules of an element (H2), which is hydrogen found in its natural state.

• Could mean atoms of an element are present in some form (sodium found in the human body).

• Look at each particular case to determine its proper use.

How the Term Element is Used

Symbols for the Elements

Section 4.2


• Each element has a unique one- or two-letter symbol.

• First letter is always capitalized and the second is not.

• The symbol usually consists of the first one or two letters of the element’s name.

Examples:Oxygen OKrypton Kr

• Sometimes the symbol is taken from the element’s original Latin or Greek name.

Examples:Gold Au aurumLead Pb plumbum

Symbols for the Elements

Section 4.2


Names and Symbols of the Most Common Elements

Dalton’s Atomic Theory

Section 4.3


1. Most natural materials are mixtures of pure substances.

2. Pure substances are either elements or combinations of elements called compounds.

3. A given compound always contains the same proportions (by mass) of the elements.


Section 4.3


• A given compound always has the same composition, regardless of where it comes from.

Water always contains 8 g of oxygen for every 1 g of hydrogen.

Carbon dioxide always contains 2.7 g of oxygen for every 1 g of carbon.

Law of Constant Composition


Section 4.3


1. Elements are made of tiny particles called atoms.

Dalton’s Atomic Theory (1808)


Section 4.3


2. All atoms of a given element are identical.

Dalton’s Atomic Theory (continued)


Section 4.3


3. The atoms of a given element are different from those of any other element.



Section 4.3


4. Atoms of one element can combine with atoms of other elements to form compounds. A given compound always has the same relative numbers and types of atoms.



Section 4.3


5. Atoms are indivisible in chemical processes. Atoms are not created or destroyed in chemical reactions. A chemical reaction simply changes the way the atoms are grouped together.



Section 4.3


Concept Check

Which of the following statements regarding Dalton’s atomic theory are still believed to be true?

I. Elements are made of tiny particles called atoms.

II. All atoms of a given element are identical.

III. A given compound always has the same relative

numbers and types of atoms.

IV. Atoms are indestructible.

Formulas of Compounds

Section 4.4


• Compound – distinct substance that is composed of the atoms of two or more elements and always contains exactly the same relative masses of those elements.

• Chemical Formulas – expresses the types of atoms and the number of each type in each unit (molecule) of a given compound.

Chemical Formulas Describe Compounds


Section 4.4


1. Each atom present is represented by its element symbol.

2. The number of each type of atom is indicated by a subscript written to the right of the element symbol.

3. When only one atom of a given type is present, the subscript 1 is not written.

Rules for Writing Formulas


Section 4.4


Exercise

The pesticide known as DDT paralyzes insects by binding to their nerve cells, leading to uncontrolled firing of the nerves. Before most uses of DDT were banned in the U.S., many insects had developed a resistance to it. Write out the formula for DDT. It contains 14 carbon

atoms, 9 hydrogen atoms, and 5 atoms of chlorine.

C14H9Cl5

The Structure of the Atom

Section 4.5


• Postulated the existence of electrons using cathode-ray tubes.

• The atom must also contain positive particles that balance exactly the negative charge carried by particles that we now call electrons.

J. J. Thomson (1898—1903)


Section 4.5


Cathode-Ray Tube


Section 4.5


William Thomson (Plum Pudding Model)

• Reasoned that the atom might be thought of as a uniform “pudding” of positive charge with enough negative electrons scattered within to counterbalance that positive charge.


Section 4.5


• Explained the nuclear atom.

• Atom has a dense center of positive charge called the nucleus.

• Electrons travel around the nucleus at a relatively large distance.

• A proton has the same magnitude of charge as the electron, but its charge is positive.

Ernest Rutherford (1911)


Section 4.5


• Most nuclei also contain a neutral particle called the neutron.

• A neutron is slightly more massive than a proton but has no charge.

Rutherford and Chadwick (1932)

Introduction to the Modern Concept of Atomic Structure

Section 4.6


The atom contains:

• Electrons – found outside the nucleus; negatively charged

• Protons – found in the nucleus; positive charge equal in magnitude to the electron’s negative charge

• Neutrons – found in the nucleus; no charge; virtually same mass as a proton


Section 4.6


• The nucleus is:

Small compared with the overall size of the atom.

Extremely dense; accounts for almost all of the atom’s mass.


Section 4.6



Section 4.6


• The chemistry of an atom arises from its electrons.

• Electrons are the parts of atoms that “intermingle” when atoms combine to form molecules.

• It is the number of electrons that really determines chemical behavior.

Why do different atoms have different chemical properties?

Isotopes

Section 4.7


• Atoms with the same number of protons but different numbers of neutrons.

• Show almost identical chemical properties; chemistry of atom is due to its electrons.

• In nature most elements contain mixtures of isotopes.

Isotopes

Isotopes

Section 4.7


Two Isotopes of Sodium

Isotopes

Section 4.7


• X = the symbol of the element

• A = the mass number (# of protons and neutrons)

• Z = the atomic number (# of protons)

Isotopes

XAZ

Isotopes

Section 4.7


Isotopes – An Example

• C = the symbol for carbon

• 6 = the atomic number (6 protons)

• 14 = the mass number (6 protons and 8 neutrons)

• C = the symbol for carbon

• 6 = the atomic number (6 protons)

• 12 = the mass number (6 protons and 6 neutrons)

146C 12

6C

Isotopes

Section 4.7


Exercise

A certain isotope X contains 23 protons and 28 neutrons.

• What is the mass number of this isotope?

• Identify the element.

Mass Number = 51

Vanadium

Introduction to the Periodic Table

Section 4.8


• The periodic table shows all of the known elements in order of increasing atomic number.

The Periodic Table


Section 4.8


• Metals vs. Nonmetals

• Groups or Families – elements in the same vertical columns; have similar chemical properties

• Periods – horizontal rows of elements

The Periodic Table


Section 4.8


• Most elements are metals and occur on the left side.

• The nonmetals appear on the right side.

• Metalloids are elements that have some metallic and some nonmetallic properties.

The Periodic Table


Section 4.8


1. Efficient conduction of heat and electricity

2. Malleability (they can be hammered into thin sheets)

3. Ductility (they can be pulled into wires)

4. A lustrous (shiny) appearance

Physical Properties of Metals


Section 4.8


1. Lack properties of metals

2. Exhibit much variation in properties

3. Can be gases, liquids, or solids

Physical Properties of Nonmetals


Section 4.8


1. Exhibit a mixture of metallic and non-metallic properties

Physical Properties of Metalloids

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